All Questions
Tagged with equilibrium aqueous-solution
20
questions
9
votes
4
answers
4k
views
Why does the inverse relationship between the strengths of an acid and its conjugate base appear to be violated in the case of chloric(I) acid?
Hypochlorous acid is a weak acid with $\mathrm{p}K_\mathrm{a}(\ce{HClO}) = 7.53$. Then why is its conjugate base, $\ce{ClO-}$, a weak base in water? Shouldn't the strength of the base be inversely ...
- 205
4
votes
1
answer
1k
views
How do I quantify the carbonate system and its pH speciation?
I did Environmental Water Chemistry as part of my undergraduate course where we quantified pH-speciation for the full carbonate system and I got it right according to my tutor. My speciation profile ...
- 500
26
votes
4
answers
3k
views
What software can calculate aqueous solution equilibria?
What software is available out there to calculate the equilibrium in a set of reactions in aqueous solution? In particular, I'm interested in software general enough to simulate things like titration ...
- 23.8k
5
votes
2
answers
3k
views
Calculating approximate pH of polyprotic acids
When I took up ionic equilibria and titrations after a long break, I found it hard to solve the questions regarding pH calculations of polyprotic acds. Consider these two questions as examples:-
...
- 6,795
4
votes
2
answers
4k
views
Dangers of expired bleach?
I have some unopened Clorox bleach bought over a year ago (at $8.25~\%\ \ce{NaOCl}$) and read on Wikipedia that bleach naturally decomposes according to
$$\ce{3 NaOCl (aq) -> NaClO3 (aq) + 2 NaCl(...
- 1,556
2
votes
1
answer
987
views
How to calculate molar concentration from equilibrium equations with no initial concentration given?
I have the equations:
\begin{align}
\ce{CO2(g) + H2O(l) &<=> H2CO3(aq)} &\quad K_1 &= 10^{-1.47} \tag{1}\\
\ce{H2CO3(aq) &<=> H+(aq) + HCO3-(aq)} &\quad K_2 &= 10^{-...
- 51
13
votes
2
answers
8k
views
Why does the ionic product of water remain constant after addition of non-neutral solute?
In my textbook, it is given that the ionic product of water $K_\mathrm{w}$ remains constant even when a non-neutral solute such as an acid is added to it.
$$K_\mathrm{w} = \ce{[H3O+][OH-]}$$
When a ...
- 295
6
votes
2
answers
25k
views
How much carbonation is in one liter of commercial fountain Coca-Cola
From what I understand generally Coke is carbonated to roughly 6.2 g per liter in bottles and cans, or 3.1 volumes of CO2. I was watching this video because I was curious about how fountain soda ...
- 131
6
votes
1
answer
7k
views
Difference in calculated pH and the real pH of a phosphate buffer
I want to prepare a buffer system with $\mathrm{pH} = 7.00$ and a total concentration $c_\mathrm{tot} = \pu{0.10 mol l^-1}$ using sodium hydrogen phosphate $(\ce{Na2HPO4})$ and sodium dihydrogen ...
- 71
4
votes
2
answers
3k
views
Why is water ignored in the ionic equilibrium of HF?
While trying to understand the solution of a problem given in my textbook, I realized I'm having some difficulty with the solution. The problem is as follows:
The ionization constant of $\ce{HF}$ ...
- 261
3
votes
1
answer
1k
views
Predicting pH of an acidic salt of an weak acid and weak base
Suppose we want to calculate pH of an $\ce{NH4HCO3}$ solution of known concentration.
Now, $\ce{NH4+}$ will be hydrolised to give $\ce{H+}$ ions.
Some $\ce{HCO3-}$ ions will be converted to (i) $\ce{...
3
votes
2
answers
5k
views
Why doesn't a buffer solution change ph(Appreciably?)
Consider a buffer solution containing weak acid $\ce{CH3COOH}$ and its salt $\ce{CH3COONa}$:
\begin{align}
\ce{CH3COOH &<=> CH3COO- + H+} \tag{1}\\
\ce{CH3COONa &-> CH3COO- + Na+} \...
- 4,197
2
votes
2
answers
28k
views
What are the effects of adding water to a system at equilibrium?
Given the reaction $\ce{NaCl~(s) <=> Na+~(aq) + Cl^{-}~(aq)}$. $\ce{NaCl}$ is added to water and equilibrium is reached.
Does the reaction shift to the left/right/not shift at all if more ...
- 53
2
votes
2
answers
345
views
Calculating equilibrium concentrations of silver and halide ions
$\pu{500 ml}$ of $\pu{0.01 M}$ $\ce{AgNO3}$ is mixed with $\pu{500 ml}$ of solution containing $\pu{0.1 M}$ $\ce{NaCl}$ and $\pu{0.1 M}$ $\ce{NaBr}$. $K_\mathrm{sp}$ of $\ce{AgCl}$ is $10^{-10}$ and $...
- 224
2
votes
1
answer
1k
views
Why degree of dissociation/ionisation affected by dilution? [closed]
What happens when we dilute, say, an acid which is weak, and then add water to it? What motivates or pushes it to dissociate more?
We are just adding some molecules of water, right? So, what exactly ...
